Chemical Kinetics. System LENGTH: VOLUME MASS Temperature. 1 gal = 4 qt. 1 qt = in 3. 1 L = qt. 1 qt = L
|
|
- Kerry Stafford
- 5 years ago
- Views:
Transcription
1 Chemical Kinetics Practice Exam Chemical Kinetics Name (last) (First) Read all questions before you start. Show all work and explain your answers to receive full credit. Report all numerical answers to the proper number of significant figures. By signing your signature above you agree that you have worked alone and neither give nor received help from any source. Keep your eyes on your own paper at all times System LENGTH: VOLUME MASS Temperature English: 1 ft = 12 in 1 gal = 4 qt 1 lb = 16 oz T F = 1.8T C mile = 5280 ft 1 qt = in 3 1 ton = 2000 lb 1 yd = 3 ft SI- English: 1 in = 2.54 cm 1 mi = km 1 L = qt 1 qt = L 1 lb = g 1 oz = g T C = (T F 32) 1.8 Misc. info 1 mole = R = J/ mol K or L atm/mol K Rates of Reaction rate = Δ[A] /Δ t = - Δ [react] /Δ t = Δ [prod] /Δ t Rate laws (Order of reaction) initial rate = k [A] x [B] y [C] z... Overall order = x + y + z +... Conc. vs. Time dependence Zeroth Order Conc. vs. Time straight line. rate = k [A] = [A]o - kt Half life; t1/2 = [A]o / 2 k First Order [A] = [A]o exp{- kt) ln[conc.] vs. Time straight line rate = k [A] ln[a] = ln[a]o - kt Half life; t1/2 = / k Second Order 1/[Conc.] vs. Time straight line rate = k [A] 2 or k [A] [B] 1/[A] = 1/[A]o + kt Half life; t1/2 = 1 / k [A]o Temperature vs. Rate dependence k = A exp {-E a /RT} ln k = ln A - (E a / R) 1/T ln(k) vs. 1/T straight line. ln(k 1/k 2) = (E a / R) (1/T 2-1/T 1)
2 Multiple -choice. Show work for partial credit. 1 Which of the following statement is true? a) The activation energy of a reaction increases with increasing temperature. b) The slowest step in a mechanism will always determine the rate of a reaction. c) A catalyst not only changes the activation energy of a reaction, it also changes ΔH rxn. d) All of these statements are true. 2 A plot of [A] -1 vs., time is most likely a a) Arrhenius equation b) second order reaction c) first order reaction d) zeroth order reaction 3 If the heat of reaction is endothermic, which of the following is always true? a ) the reaction is fast b) the reaction is slow c) the energy of the reactants is greater than the products d) the energy of the reactants is lower than the products 4 The rate of a reaction is not influenced by: a) concentration of reactant b) Catalyst c) Energy of Reactant d) stirring of chemicals 5 The pre-exponential factor in the Arhenius equation takes in to account: a) The steric factor b) The activation energy c) The energy of the reaction d) The Maxwell-Boltzmann curve.
3 6 The reaction: 2I - (aq) + S2O8 2- (aq) I2(aq) + 2SO4 2- (aq) was studied at 25 C. The following results were obtained [ I - ] o (M) [S2O8 2- ] (M) Initial Rate (M/s) i) Determine the rate law. i) Rate = k [I ] x [S 2 O 8 2 ] y = k [I ] 0 [S 2 O 8 2 ] 2 ii) What is the rate constant using experiment # 2 iii) What is the molecularity of this reaction? iv) Calculate the half-life using the data from Experiment2 Rate(expt2) = k [I ] 0 [S 2 O 8 2 ] 2 ii) = k [.040] 0 [.040] 2 k = 3.125x [.040] 2 = iii) Bimolecular since Order = 2 = iv) 1 t 12 = k A o [ ] = [.040M] =12,800 s 7 Determine if the statements below are true or false then write a convincing statement to justify your answer. a) At a given temperature, all molecules posses the same kinetic energy False. The MB distribution plot shows that any given temperature molecules will have a range of kinetic energy with the average centered at the U rms. b) Reactant molecules must collide with greater energy than the activation energy in order to change to product molecules. False. Not only must the molecules collide with sufficient energy to overcome the activation energy, they molecules must also have the right orientation (steric factor). c) The activation energy of a reaction is not dependent on the temperature. True. The E act is a function of the mechanism of the reaction, which is a function of the chemicals that are involve in the reaction. Remember in the Crystal Violet Experiment that E act was the same whether the data was collected at high temperature or low temperature. In fact the temperature data was used to determine E act. d) A catalyst increases the rate by increasing collision frequency. False. A catalyst changes the mechanism, which alters (lowering) the Eact, thereby increasing the rate of the reaction. The reason the reaction rate increases is because Eact decreases. Collision Frequency may have been altered but it is not the primary reason for the rate change. 8 Explain using a Maxwell-Boltzmann Distribution curve why an exothermic reaction favors an increase of the reverse reaction at higher temperature even though according to the Kinetic Molecular Theory, the rate of a reaction increases with increasing temperature. For an exothermic reaction, if the temperature is increase, the percentage of the product molecules is greater than that of the reactant that surpasses the activation Energy. Therefore more products will return to reactants therefore shifting the reaction to the left.
4 9 Most reaction occurs by a series of steps. The energy profile shown below is a three-step mechanism for the reaction of NO with H2. i) 2NO N 2 O 2 fast ΔH 1 = + 20 kj Eact 1 = 50 kj E 1 = 50 kj (Transition state) ii) N 2 O 2 + H 2 N2O + H2O slow ΔH 2 = + 30 kj Eact 2 = E 2 = 100 kj iii) N2O + H 2 N 2 + H2O fast ΔH 3 = - 10 kj Eact 3 = 30 kj E 3 =? Place answers to questions ii, iii, iv, & vi. E (NO) = 0_kJ E(N 2 O 2 )= 20 kj Eact2 = 80 kj E 3 = 80 kj ΔHrxn= 40 kj Eact(f)= 100 kj Eact(r)= 60 kj Label the graph above placing the chemical specie along the reaction profile diagram and then answer the following: i) What is the overall stoichiometry and what are the intermediate and the catalyst (if any)? 2NO + 2H 2 N 2 + 2H 2 O, Intermediate = N 2 O 2, N 2 O, Catalyst = None ii) What are the energies of NO and N2O2 according to the graph above? E NO = 0 kj E N2O 2 = 20 kj iii) What are the energies of Eact2 and E 3? Eact2 = 80 kj E 3 = 80 kj iv) What is the energy of the overall reaction, DHrxn? ΔHrxn = + 40 kj v) Is the reaction endothermic or exothermic? ΔHrxn = + 40 kj > 0, Endothermic vi) What are the activation energies for the overall forward Eact(f), and overall reverse Eact(r), reactions? Eact(f) = 100 kj E act(r) = 60 kj vii) What are the rate law and the molecularity for this reaction? Rate = k [N 2 O 2 ] [H 2 ], but N 2 O 2 is an intermediate thus K eq = [N 2 O 2 ] / [NO] 2 Thus, Rate = k Keq [NO] 2 * [H 2 ] = K [NO] 2 * [H 2 ], termolecular viii) If the pre-exponential factor is , what is the rate constant (include units) for this reaction at 600K? k = A exp [-E a /RT}, thus k = exp [-100,000 J / J mol K -1 * 600 K} k = 25 M -2 / s ix) What temperature is required to raise the rate constant to 250? (units are not shown here) k = A exp [-E a /RT}, lnk = lna - E a /RT, T = E a /R(lnK lna), T = 678 K x) If the catalyzed reaction is ten times faster than the uncatalyzed reaction, what is the rate of disappearance of the reactant for the catalyzed reaction? You may assume that you are using the methods of initial rates in which the concentration of all chemicals are 1.0 M. T= 600 K Rate = 250 M / s
5 10 The reaction of hydrogen with iodine has the following accepted mechanism: (1) I2 (g) 2I (g) fast (2) H2(g) + I (g) H2I (g) fast (3) H2I (g) + I (g) 2HI (g) slow What is the rate law for this reaction? 11 Consider the following reaction energy diagram: i) How many elementary steps in the reaction mechanism? 170 kj A C ii) Which step is rate limiting? i.e. 1st, 2nd, 3rd, 4th,... iii) Is the overall reaction exothermic or endothermic? iv) What is the energy of the reaction (kj)? v) What is the activation energy (kj) for the reverse rxn? 100 kj 45 kj 0 kj - 60 kj A B C vi) What is the Eact (kj) for the rate determining step?
6 12 A theoretical reaction: A + B C, has the following initial rate data shown below. Expt. # [A] M [B] M -Δ [A] / Δt M/s 1 (300K) x (300K) x (300K) x (300K) x (600K) i) Determine the complete rate law for the reaction including the rate constant with proper units. ii) What is the activation energy (Ea in kj) for this reaction and the frequency factor (A).
7 13 A slightly bruised apple will rot extensively in about 4 days at room temperature (20 C). If it is kept in the refrigerator at 0 C, the same extent of rotting takes about 16 days. What is the Eact (kj) for the rotting reaction?
8 14 Determine if the statements are true or false. Give a reasonable explanation to support or refute these statements. i) At a given temperature, all molecules posses the same kinetic energy. ii) The higher the activation energy of a reaction, the slower the rate of the reaction. iii) If reactant molecules collide with greater energy than the activation energy, products are formed automatically. iv) Exothermic reaction have faster rates than endothermic reactions. v) The activation energy of a reaction is lowered by a catalyst. vi) The enthalpy change for a reaction is lowered by a catalyst
1.8. ΔG = ΔH - TΔS ΔG = ΔG + RT ln Q ΔG = - RT ln K eq. ΔX rxn = Σn ΔX prod - Σn ΔX react. ΔE = q + w ΔH = ΔE + P ΔV ΔH = q p = m Cs ΔT
ThermoDynamics Practice Exam Thermodynamics Name (last) (First) Read all questions before you start. Show all work and explain your answers to receive full credit. Report all numerical answers to the proper
More information1.8. ΔG = ΔH - TΔS ΔG = ΔG + RT ln Q ΔG = - RT ln K eq. ΔX rxn = Σn ΔX prod - Σn ΔX react. ΔE = q + w ΔH = ΔE + P ΔV ΔH = q p = m Cs ΔT
ThermoDynamics Practice Exam Thermodynamics Name (last) (First) Read all questions before you start. Show all work and explain your answers to receive full credit. Report all numerical answers to the proper
More informationAP CHEMISTRY CHAPTER 12 KINETICS
AP CHEMISTRY CHAPTER 12 KINETICS Thermodynamics tells us if a reaction can occur. Kinetics tells us how quickly the reaction occurs. Some reactions that are thermodynamically feasible are kinetically so
More information3: Chemical Kinetics Name: HW 6: Review for Unit Test KEY Class: Date: A Products
3: Chemical Kinetics Name: HW 6: Review for Unit Test KEY Class: Date: Page 1 of 9 AP Multiple Choice Review Questions 1 16 1. The reaction rate is defined as the change in concentration of a reactant
More informationCh 13 Rates of Reaction (Chemical Kinetics)
Ch 13 Rates of Reaction (Chemical Kinetics) Reaction Rates and Kinetics - The reaction rate is how fast reactants are converted to products. - Chemical kinetics is the study of reaction rates. Kinetics
More informationHomework 07. Kinetics
HW07 - Kine!cs Started: Mar at 10:56am Quiz Instruc!ons Homework 07 Kinetics Question 1 Consider the reaction: O (g) 3O (g) rate = k[o ] [O ] 3 3 What is the overall order of the reaction and the order
More informationChemical Kinetics -- Chapter 14
Chemical Kinetics -- Chapter 14 1. Factors that Affect Reaction Rate (a) Nature of the reactants: molecular structure, bond polarity, physical state, etc. heterogeneous reaction: homogeneous reaction:
More informationKEY for CHEM 116 EXAM #2 PRACTICE
Circle the correct answers ( points each) KEY for CHEM 6 EXAM # PRACTICE. If the half-life of a reaction depends on the concentration of the reactant, then the reaction cannot be order. a. second b. zero
More informationChapter 12. Chemical Kinetics
Chapter 12 Chemical Kinetics Chapter 12 Table of Contents 12.1 Reaction Rates 12.2 Rate Laws: An Introduction 12.3 Determining the Form of the Rate Law 12.4 The Integrated Rate Law 12.5 Reaction Mechanisms
More informationQuadratic Equation: ax 2 + bx + c = 0
Exam # Key (last) (First-Name) Signature Exam 2 General Chemistry 201. May 12, 2009 No credit will be given for correct numerical answers without a clear indication of how they were obtained. Show all
More informationChemical Kinetics. Chapter 13. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chemical Kinetics Chapter 13 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does
More informationCHAPTER 13 (MOORE) CHEMICAL KINETICS: RATES AND MECHANISMS OF CHEMICAL REACTIONS
CHAPTER 13 (MOORE) CHEMICAL KINETICS: RATES AND MECHANISMS OF CHEMICAL REACTIONS This chapter deals with reaction rates, or how fast chemical reactions occur. Reaction rates vary greatly some are very
More informationB. Activation Energy: Ea
B. Activation Energy: Ea a) Example reaction: the burning of charcoal in the BBQ C (s) + O 2(g) CO 2 (remember, burning is VERY exothermic) Question: Will charcoal in your BBQ spontaneously catch fire?
More informationChapter 11 Rate of Reaction
William L Masterton Cecile N. Hurley http://academic.cengage.com/chemistry/masterton Chapter 11 Rate of Reaction Edward J. Neth University of Connecticut Outline 1. Meaning of reaction rate 2. Reaction
More informationYes. Yes. Yes. Experimental data: the concentration of a reactant or product measured as a function of time. Graph of conc. vs.
Experimental data: the concentration of a reactant or product measured as a function of time Graph of conc. vs. time Is graph a straigh t line? No Graph of ln[conc.] vs. time Yes System is zero order Is
More informationFactors That Affect Rates. Factors That Affect Rates. Factors That Affect Rates. Factors That Affect Rates
KINETICS Kinetics Study of the speed or rate of a reaction under various conditions Thermodynamically favorable reactions DO NOT mean fast reactions Some reactions take fraction of a second (explosion)
More informationAP CHEMISTRY NOTES 7-1 KINETICS AND RATE LAW AN INTRODUCTION
AP CHEMISTRY NOTES 7-1 KINETICS AND RATE LAW AN INTRODUCTION CHEMICAL KINETICS the study of rates of chemical reactions and the mechanisms by which they occur FACTORS WHICH AFFECT REACTION RATES 1. Nature
More informationRates, Temperature and Potential Energy Diagrams Worksheet
SCH4U1 ER10 Name: Date: Rates, Temperature and Potential Energy Diagrams Worksheet Part 1: 1. Use the potential energy diagram shown to the right to answer the following: a. Label the axis. y axis is potential
More informationChapter 13 Kinetics: Rates and Mechanisms of Chemical Reactions
Chapter 13 Kinetics: Rates and Mechanisms of Chemical Reactions 14.1 Focusing on Reaction Rate 14.2 Expressing the Reaction Rate 14.3 The Rate Law and Its Components 14.4 Integrated Rate Laws: Concentration
More informationChapter 12. Chemical Kinetics
Chapter 12 Chemical Kinetics Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section
More informationChemical Kinetics Ch t ap 1 er
Chemical Kinetics Chapter 13 1 Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does a reaction proceed? Reaction rate is the change in the concentration of a reactant or
More informationChapter 12 - Chemical Kinetics
Chapter 1 - Chemical Kinetics 1.1 Reaction Rates A. Chemical kinetics 1. Study of the speed with which reactants are converted to products B. Reaction Rate 1. The change in concentration of a reactant
More informationIt must be determined from experimental data, which is presented in table form.
Unit 10 Kinetics The rate law for a reaction describes the dependence of the initial rate of a reaction on the concentrations of its reactants. It includes the Arrhenius constant, k, which takes into account
More informationAP Chemistry - Notes - Chapter 12 - Kinetics Page 1 of 7 Chapter 12 outline : Chemical kinetics
AP Chemistry - Notes - Chapter 12 - Kinetics Page 1 of 7 Chapter 12 outline : Chemical kinetics A. Chemical Kinetics - chemistry of reaction rates 1. Reaction Rates a. Reaction rate- the change in concentration
More informationChemical Kinetics. What quantities do we study regarding chemical reactions? 15 Chemical Kinetics
Chemical Kinetics Chemical kinetics: the study of reaction rate, a quantity conditions affecting it, the molecular events during a chemical reaction (mechanism), and presence of other components (catalysis).
More informationChemical Kinetics. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chemical Kinetics Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does a reaction
More informationReaction Rate. Rate = Conc. of A at t 2 -Conc. of A at t 1. t 2 -t 1. Rate = Δ[A] Δt
Kinetics The study of reaction rates. Spontaneous reactions are reactions that will happen - but we can t tell how fast. Diamond will spontaneously turn to graphite eventually. Reaction mechanism- the
More informationChapter 11: CHEMICAL KINETICS
Chapter : CHEMICAL KINETICS Study of the rate of a chemical reaction. Reaction Rate (fast or slow?) Igniting gasoline? Making of oil? Iron rusting? We know about speed (miles/hr). Speed Rate = changes
More informationCh 13 Chemical Kinetics. Modified by Dr. Cheng-Yu Lai
Ch 13 Chemical Kinetics Modified by Dr. Cheng-Yu Lai Outline 1. Meaning of reaction rate 2. Reaction rate and concentration 3. Writing a Rate Law 4. Reactant concentration and time 5. Reaction rate and
More informationChem 401 Unit 1 (Kinetics & Thermo) Review
KINETICS 1. For the equation 2 H 2(g) + O 2(g) 2 H 2 O (g) How is the rate of formation of H 2 O mathematically related to the rate of disappearance of O 2? 1 Δ [H2O] Δ[O 2] = 2 Δt Δt 2. Determine the
More informationconcentrations (molarity) rate constant, (k), depends on size, speed, kind of molecule, temperature, etc.
#73 Notes Unit 9: Kinetics and Equilibrium Ch. Kinetics and Equilibriums I. Reaction Rates NO 2(g) + CO (g) NO (g) + CO 2(g) Rate is defined in terms of the rate of disappearance of one of the reactants,
More informationCHAPTER 12 CHEMICAL KINETICS
5/9/202 CHAPTER 2 CHEMICAL KINETICS CHM52 GCC Kinetics Some chemical reactions occur almost instantaneously, while others are very slow. Chemical Kinetics - study of factors that affect how fast a reaction
More informationExam I Solutions Chem 6, 9 Section, Spring 2002
1. (a) Two researchers at the University of Nebraska recently published a paper on the rate of the disappearance of World Wide Web links, a phenomenon called link rot. They asked the question, If I place
More informationChemistry 102 Chapter 14 CHEMICAL KINETICS. The study of the Rates of Chemical Reactions: how fast do chemical reactions proceed to form products
CHEMICAL KINETICS Chemical Kinetics: The study of the Rates of Chemical Reactions: how fast do chemical reactions proceed to form products The study of Reaction Mechanisms: the steps involved in the change
More information1 A burning splint will burn more vigorously in pure oxygen than in air because
Slide 1 / 38 1 burning splint will burn more vigorously in pure oxygen than in air because oxygen is a reactant in combustion and concentration of oxygen is higher in pure oxygen than is in air. oxygen
More informationChapter 14 Chemical Kinetics
7/10/003 Chapter 14 Chemical Kinetics 14-1 Rates of Chemical Reactions 14- Reaction Rates and Concentrations 14-3 The Dependence of Concentrations on Time 14-4 Reaction Mechanisms 14-5 Reaction Mechanism
More informationNAME: Chapter 14Chemical Kinetics (Reaction Rate Law Concepts)
NAME: Chapter 14Chemical Kinetics (Reaction Rate Law Concepts) 1. Go to the website : http://www.chm.davidson.edu/vce/kinetics/index.html, a. Go to reaction rates page, read the introductory paragraphs
More informationHow can we use the Arrhenius equation?
How can we use the Arrhenius equation? k = Ae Ea RT Lab H 3 CNC(g) H 3 CCN(g) 1. Experiment to determine rate law 2. Experiment to determine Ea Temperature (K) k (s -1 ) 1/T ln k 462.9 2.52E-05 0.00216-10.589
More informationEnergy Changes, Reaction Rates and Equilibrium. Thermodynamics: study of energy, work and heat. Kinetic energy: energy of motion
Energy Changes, Reaction Rates and Equilibrium Thermodynamics: study of energy, work and heat Kinetic energy: energy of motion Potential energy: energy of position, stored energy Chemical reactions involve
More informationC H E M I C N E S C I
C H E M I C A L K I N E T S C I 4. Chemical Kinetics Introduction Average and instantaneous Rate of a reaction Express the rate of a reaction in terms of change in concentration Elementary and Complex
More informationCHAPTER 17 REVIEW. Reaction Kinetics. Answer the following questions in the space provided. Energy B A. Course of reaction
CHAPTER 17 REVIEW Reaction Kinetics SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Refer to the energy diagram below to answer the following questions. D Energy C d c d
More informationChapter 12. Chemical Kinetics
Chapter 12 Chemical Kinetics Section 12.1 Reaction Rates Reaction Rate Change in concentration of a reactant or product per unit time. Rate = concentration of A at time t t 2 1 2 1 concentration of A at
More informationCollision Theory. and I 2
Collision Theory To explain why chemical reactions occur, chemists have proposed a model, known as collision theory, which states that molecules must collide in order to react. These collisions can involve
More informationChapter 14: Chemical Kinetics II. Chem 102 Dr. Eloranta
Chapter 14: Chemical Kinetics II Chem 102 Dr. Eloranta Rate Laws If you are familiar with calculus Experiments would allow you to determine the reaction order and rate constant, but what if you wanted
More informationChemical Kinetics. Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions:
Chemical Kinetics Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions: reactant concentration temperature action of catalysts surface
More informationName: UNIT 5 KINETICS NOTES PACEKT #: KINETICS NOTES PART C
KINETICS NOTES PART C IV) Section 14.4 The Change of Concentration with Time A) Integrated Rate Law: shows how the concentration of the reactant(s) varies with time 1) [A]0 is the initial concentration
More informationChapter 14 Chemical Kinetics
4//004 Chapter 4 Chemical Kinetics 4- Rates of Chemical Reactions 4- Reaction Rates and Concentrations 4-3 The Dependence of Concentrations on Time 4-4 Reaction Mechanisms 4-5 Reaction Mechanism and Rate
More informationChemical Kinetics. Rate = [B] t. Rate = [A] t. Chapter 12. Reaction Rates 01. Reaction Rates 02. Reaction Rates 03
Chapter Chemical Kinetics Reaction Rates 0 Reaction Rate: The change in the concentration of a reactant or a product with time (M/s). Reactant Products aa bb Rate = [A] t Rate = [B] t Reaction Rates 0
More informationChapter 14: Chemical Kinetics
Chapter 14: Chemical Kinetics NOTE THIS CHAPTER IS #2 TOP TOPICS ON AP EXAM!!! NOT ONLY DO YOU NEED TO FOCUS ON THEORY (and lots of MATH) BUT YOU MUST READ THE FIGURES TOO!!! Ch 14.1 ~ Factors that Affect
More informationCHEMISTRY. Chapter 14 Chemical Kinetics
CHEMISTRY The Central Science 8 th Edition Chapter 14 Kozet YAPSAKLI kinetics is the study of how rapidly chemical reactions occur. rate at which a chemical process occurs. Reaction rates depends on The
More informationKINETICS CHEMICAL CHEMIC. Unit. I. Multiple Choice Questions (Type-I)
Unit 4 CHEMICAL CHEMIC KINETICS I. Multiple Choice Questions (Type-I) 1. The role of a catalyst is to change. gibbs energy of reaction. enthalpy of reaction. activation energy of reaction. equilibrium
More information3. A forward reaction has an activation energy of 50 kj and a H of 100 kj. The PE. diagram, which describes this reaction, is
Kinetics Quiz 4 Potential Energy Diagrams 1. A catalyst increases the rate of a reaction by A. Increasing the concentration of the reactant(s) B. Decreasing the concentration of the reactant(s) C. Increasing
More informationCollision Theory. Unit 12: Chapter 18. Reaction Rates. Activation Energy. Reversible Reactions. Reversible Reactions. Reaction Rates and Equilibrium
Collision Theory For reactions to occur collisions between particles must have Unit 12: Chapter 18 Reaction Rates and Equilibrium the proper orientation enough kinetic energy See Both In Action 1 2 Activation
More informationAP Questions: Kinetics
AP Questions: Kinetics 1972 2 A + 2 B C + D The following data about the reaction above were obtained from three experiments: Rate of Formation of [A] [B] C (mole. liter -1 min -1 ) 1 0.60 0.15 6.3 10-3
More information11/9/2012 CHEMICAL REACTIONS. 1. Will the reaction occur? 2. How far will the reaction proceed? 3. How fast will the reaction occur?
CHEMICAL REACTIONS LECTURE 11: CHEMICAL KINETICS 1. Will the reaction occur? 2. How far will the reaction proceed? 3. How fast will the reaction occur? CHEMICAL REACTIONS C(s, diamond) C(s, graphite) G
More informationHomework #4 Chapter 15 Chemical Kinetics. Therefore, k depends only on temperature. The rate of the reaction depends on all of these items (a d).
Homework #4 Chapter 5 Chemical Kinetics 8. Arrhenius Equation Therefore, k depends only on temperature. The rate of the reaction depends on all of these items (a d). 4. a) d) b) c) e) 5. Rate has units
More informationREACTION KINETICS. Catalysts substances that increase the rates of chemical reactions without being used up. e.g. enzymes.
REACTION KINETICS Study of reaction rates Why? Rates of chemical reactions are primarily controlled by 5 factors: the chemical nature of the reactants 2 the ability of the reactants to come in contact
More informationCHEMISTRY - CLUTCH CH.13 - CHEMICAL KINETICS.
!! www.clutchprep.com CONCEPT: RATES OF CHEMICAL REACTIONS is the study of reaction rates, and tells us the change in concentrations of reactants or products over a period of time. Although a chemical
More informationCHEM Chapter 14. Chemical Kinetics (Homework) Ky40
CHEM 1412. Chapter 14. Chemical Kinetics (Homework) Ky40 1. Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2ClO 2 (aq) + 2OH (aq) ClO
More informationChapter 14. Chemical Kinetics
Chapter 14. Chemical Kinetics Common Student Misconceptions It is possible for mathematics to get in the way of some students understanding of the chemistry of this chapter. Students often assume that
More informationCHEM Dr. Babb s Sections Lecture Problem Sheets
CHEM 116 - Dr. Babb s Sections Lecture Problem Sheets Kinetics: Integrated Form of Rate Law 61. Give the integrated form of a zeroth order reaction. Define the half-life and find the halflife for a general
More informationName AP CHEM / / Chapter 12 Outline Chemical Kinetics
Name AP CHEM / / Chapter 12 Outline Chemical Kinetics The area of chemistry that deals with the rate at which reactions occur is called chemical kinetics. One of the goals of chemical kinetics is to understand
More informationChapter 14 Chemical Kinetics
Chapter 14 Chemical Kinetics Learning goals and key skills: Understand the factors that affect the rate of chemical reactions Determine the rate of reaction given time and concentration Relate the rate
More informationExamples of fast and slow reactions
1 of 10 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly
More informationU N I T T E S T P R A C T I C E
South Pasadena AP Chemistry Name 2 Chemical Kinetics Period Date U N I T T E S T P R A C T I C E Part 1 Multiple Choice You should allocate 30 minutes to finish this portion of the test. No calculator
More informationUnit #10. Chemical Kinetics
Unit #10 Chemical Kinetics Zumdahl Chapter 12 College Board Performance Objectives: Express the rate of a reaction in terms of changes in the concentration of a reactant or a product per time. Understand
More informationChapter 12. Kinetics. Factors That Affect Reaction Rates. Factors That Affect Reaction Rates. Chemical. Kinetics
PowerPoint to accompany Kinetics Chapter 12 Chemical Kinetics Studies the rate at which a chemical process occurs. Besides information about the speed at which reactions occur, kinetics also sheds light
More informationChemical Kinetics and Equilibrium
Chemical Kinetics and Equilibrium Part 1: Kinetics David A. Katz Department of Chemistry Pima Community College Tucson, AZ USA Chemical Kinetics The study of the rates of chemical reactions and how they
More informationChapter 30. Chemical Kinetics. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.
Chapter 30 Chemical Kinetics 1 Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Chemists have three fundamental questions in mind when they study chemical reactions: 1.) What happens?
More information1. Which of the following units could be used to express the reaction rate?
Chemistry 12 Kinetics Practice Test # 2 1. Which of the following units could be used to express the reaction rate? A. ml/s B. ml/g C. g/ml D. ml/mol 2. Consider the reaction: Zn (s) + 2HCl (aq) ZnCl 2(aq)
More informationKinetics. Chapter 14. Chemical Kinetics
Lecture Presentation Chapter 14 Yonsei University In kinetics we study the rate at which a chemical process occurs. Besides information about the speed at which reactions occur, kinetics also sheds light
More informationChemical. Chapter 14. Kinetics. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E.
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 14 1 PDF Created with deskpdf PDF www.farq.xyz Writer - Trial :: http://www.docudesk.com
More informationShroud of Turin. Chemical Kinetics. Reaction Rates. Reaction Rates. Reaction Rates. Chemical Kinetics: The Rates of Chemical Reactions
Page III-12-1 / Chapter Twelve Lecture Notes Chemical Kinetics: The Rates of Chemical Reactions Chapter 12 Chemistry 222 Professor Michael Russell Shroud of Turin Shroud of Jesus?!? Fake or Real? Explored
More informationRates and Temperature
Rates and Temperature N Goalby Chemrevise.org Activation Energy Molecules will only react if they collide with enough energy to break the relevant bonds in one or either of the reactant molecules. This
More informationChapter 14 Chemical Kinetics
Chapter 14 Chemical Kinetics Factors that Affect Reaction rates Reaction Rates Concentration and Rate The Change of Concentration with Time Temperature and Rate Reactions Mechanisms Catalysis Chemical
More information11/2/ and the not so familiar. Chemical kinetics is the study of how fast reactions take place.
Familiar Kinetics...and the not so familiar Reaction Rates Chemical kinetics is the study of how fast reactions take place. Some happen almost instantaneously, while others can take millions of years.
More informationChapter 14: Chemical Kinetics
C h e m i c a l K i n e t i c s P a g e 1 Chapter 14: Chemical Kinetics Homework: Read Chapter 14 Work out sample/practice exercises in the sections, Check for the MasteringChemistry.com assignment and
More information1) a) ClO b) Cl c) O (g) + O 3(g) ---> 2O 2(g)
1) a) ClO b) Cl c) O (g) + O 3(g) ---> 2O 2(g) 2) a) D, lower concentration of reactant, decrease # of collisions. b) I, increase concentration, increase # of collisions. c) D, decrease # of collisions,
More informationLecture Presentation. Chapter 14. James F. Kirby Quinnipiac University Hamden, CT. Chemical Kinetics Pearson Education, Inc.
Lecture Presentation Chapter 14 James F. Kirby Quinnipiac University Hamden, CT In chemical kinetics we study the rate (or speed) at which a chemical process occurs. Besides information about the speed
More informationChapter 14. Chemical Kinetics
Chapter 14. Chemical Kinetics 14.1 Factors that Affect Reaction Rates The speed at which a chemical reaction occurs is the reaction rate. Chemical kinetics is the study of how fast chemical reactions occur.
More informationKinetics - Chapter 14. reactions are reactions that will happen - but we can t tell how fast. - the steps by which a reaction takes place.
The study of. Kinetics - Chapter 14 reactions are reactions that will happen - but we can t tell how fast. - the steps by which a reaction takes place. Factors that Affect Rx Rates 1. The more readily
More information10 Reaction rates and equilibrium Answers to practice questions. OCR Chemistry A. number 1 (a) 1: The enthalpy change, H;
1 (a) 1: The enthalpy change, H; 2: The activation energy, E a 1 (b) H is unaffected as it is the difference between the reactants and products E a decreases as a catalyst allows an alternative route of
More information14.1 Expressing the Reaction Rate
14.1 Expressing the Reaction Rate Differential Rate and Integrated Rate Laws Fred Omega Garces Chemistry 201 Miramar College 1 Expressing Reaction Rates Outline Kinetics: Intro Factors influencing Reaction
More informationCFC: chlorofluorocarbons
The rate of reaction is markedly affected by temperature. Chemical Kinetics & k versus T Two theories were developed to explain the temperature effects. 1. 2. 2 UV radiation strikes a CFC molecule causing
More informationChapter 14: Chemical Kinetics
1. Which one of the following units would not be an acceptable way to express reaction rate? A) M/s B) M min 1 C) L mol 1 s 1 D) mol L 1 s 1 E) mmhg/min 3. For the reaction BrO 3 + 5Br + 6H + 3Br 2 + 3H
More informationChapter 14 Chemical Kinetics
Chapter 14 14.1 Factors that Affect Reaction Rates 14.2 Reaction Rates 14.3 Concentration and Rate Laws 14.4 The Change of Concentration with Time 14.5 Temperature and Rate 14.6 Reaction Mechanisms 14.7
More informationLecture (3) 1. Reaction Rates. 2 NO 2 (g) 2 NO(g) + O 2 (g) Summary:
Summary: Lecture (3) The expressions of rate of reaction and types of rates; Stoichiometric relationships between the rates of appearance or disappearance of components in a given reaction; Determination
More informationCHEMISTRY NOTES CHEMICAL KINETICS
CHEMICAL KINETICS Rate of chemical reactions The rate of a reaction tells us how fast the reaction occurs. Let us consider a simple reaction. A + B C + D As the reaction proceeds, the concentration of
More informationChem 116 POGIL Worksheet - Week 6 Kinetics - Part 2
Chem 116 POGIL Worksheet - Week 6 Kinetics - Part 2 Why? A different form of the rate law for a reaction allows us to calculate amounts as a function of time. One variation on this gives us the concept
More informationLecture Presentation. Chapter 14. Chemical Kinetics. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.
Lecture Presentation Chapter 14 John D. Bookstaver St. Charles Community College Cottleville, MO In kinetics we study the rate at which a chemical process occurs. Besides information about the speed at
More informationKINETICS STUDY GUIDE- Written INTRODUCTION
Written Kinetics KINETICS STUDY GUIDE- Written Section: What follows is a comprehensive guide to the written component of the Chemistry 12 Provincial exam for the Unit. The questions below are from previous
More informationHow fast reactants turn into products. Usually measured in Molarity per second units. Kinetics
How fast reactants turn into products. Usually measured in Molarity per second units. Kinetics Reaction rated are fractions of a second for fireworks to explode. Reaction Rates takes years for a metal
More information1. Which of the following units could be used to express the reaction rate?
Chemistry 12 Kinetics Practice Test # 2 1. Which of the following units could be used to express the reaction rate? A. ml/s B. ml/g C. g/ml D. ml/mol 2. Consider the reaction: Zn (s) + 2HCl (aq) ZnCl 2(aq)
More informationChapter 14 Chemical Kinetics
How fast do chemical processes occur? There is an enormous range of time scales. Chapter 14 Chemical Kinetics Kinetics also sheds light on the reaction mechanism (exactly how the reaction occurs). Why
More informationLecture 19: Introduction to Kinetics First a CH 302 Kinetics Study Guide (Memorize these first three pages, they are all the background you need)
Lecture 19: Introduction to Kinetics First a CH 302 Kinetics Study Guide (Memorize these first three pages, they are all the background you need) Reaction Rate: The most important issue in kinetics is
More informationKinetics. 1. Consider the following reaction: 3 A 2 B How is the average rate of appearance of B related to the average rate of disappearance of A?
Kinetics 1. Consider the following reaction: 3 A 2 B How is the average rate of appearance of B related to the average rate of disappearance of A? A. [A]/ t = [B]/ t B. [A]/ t = (2/3)( [B]/ t) C. [A]/
More informationChapter 13 Lecture Lecture Presentation. Chapter 13. Chemical Kinetics. Sherril Soman Grand Valley State University Pearson Education, Inc.
Chapter 13 Lecture Lecture Presentation Chapter 13 Chemical Kinetics Sherril Soman Grand Valley State University Ectotherms Lizards, and other cold-blooded creatures, are ectotherms animals whose body
More informationAP * Chemistry. Kinetics: Integrated Rate Law & Determining Ea. René McCormick
AP * Chemistry Kinetics: Integrated Rate Law & Determining Ea René McCormick *AP is a registered trademark of the College Board, which was not involved in the production of, and does not endorse, this
More information